In a 500 mL flask, the degree of dissociation of PCl5 at equilibrium is 40 % and the initial amount is 5 moles. The value of equilibrium constant in mol L-1 for the decomposition of PCl5 is

Question

In a 500 mL flask, the degree of dissociation of PCl5 at equilibrium is 40 % and the initial amount is 5 moles. The value of equilibrium constant in mol L-1 for the decomposition of PCl5 is (A) 2.33 (B) 2.66 (C) 5.32 (D) 4.66

Tardigrade Admin · Accepted Answer

<img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/9cbd47e3fdec15ba873d639a0c041a1a-.png" /> α=40 % =0.4 Kc=(P C l3 Cl 2/P C l5) =((5 × 0.4/0.5 × 0.5)/(5 × 0.6)0.5)=(16/6) =2.66 mol / L

Q. In a $500 m L$ flask, the degree of dissociation of $PC l_{5}$ at equilibrium is $40%$ and the initial amount is $5$ moles. The value of equilibrium constant in $m o l L^{- 1}$ for the decomposition of $PC l_{5}$ is

2.33

2.66

5.32

4.66

$α = 40%$
$= 0.4$
$K_{c} = \frac{PC l _{3} C l _{2}}{PC l _{5}}$
$= \frac{\frac{5 \times 0.4}{0.5 \times 0.5}}{\frac{5 \times 0.6}{0.5}} = \frac{16}{6}$
$= 2.66 m o l / L$

Q. In a 500mL flask, the degree of dissociation of PCl5​ at equilibrium is 40% and the initial amount is 5 moles. The value of equilibrium constant in molL−1 for the decomposition of PCl5​ is